Thermodynamics in Chemistry Quiz

Volume is a property that depends on the size or extent of the system.

The first law states that energy in an isolated system remains constant; it cannot be created or destroyed, only converted.

Heat capacity (C) is the measure of the amount of heat required to change the temperature of a substance by 1 K.

An isochoric process is characterized by constant volume, resulting in no change in temperature.

Entropy is a thermodynamic property representing the degree of disorder or randomness in a system.

Enthalpy is a thermodynamic property that quantifies the total heat content of a system.

In an adiabatic process, there is no heat exchange with the surroundings, resulting in no change in enthalpy.

The second law relates entropy change (ΔS) to heat exchange in a reversible process (ΔS = q_rev/T).

Gibbs free energy change (ΔG) is related to enthalpy change (ΔH) and temperature (ΔS) in a system at constant temperature and pressure.

Work is not a state function; it depends on the path taken during a process rather than just the initial and final states.

The temperature at which K equals 1 depends on the specific reaction; there is no universal temperature for this condition.

An adiabatic process involves no heat exchange with the surroundings.

For a pure substance in its standard state, the entropy change is approximately zero at 298 K and 1 atm.

The standard enthalpy change for the formation of one mole of water at 25°C is -285.8 kJ/mol.

The Clausius statement emphasizes the directionality of heat flow, stating it cannot occur spontaneously from colder to hotter bodies.

At equilibrium, the standard Gibbs free energy change (∆G°) for a reaction is zero.

The change in Helmholtz free energy (∆A) is related to internal energy (∆U) and temperature (∆S) in a system.